A flexible box contains 5.60 grams of nitrogen gas (N2) which is maintained at a constant pressure of 1.35 x 105 Pa. The box is placed over a fire, causing the volume to increase from 0.00200 m³ to 0.00300 m³. Find the increase in temperature of the gas. (For N2 molar mass M = 28 grams.)

A container having a volume of 2.30 L holds 1.80 g of helium gas at a temperature of 29.0 °C. (a) Find the pressure in the container. P = atm (b) Helium behaves as an ideal monoatomic gas. Find the internal energy of the system. Eint =

A 0.75 m3 container of an ideal gas at atmospheric pressure is at a temperature of 40 oC and contains heat energy Q. The gas is heated so it now contains heat energy 1.75Q. The temperature of the gas is now

(a) After J. J. Thompson experimentally discovered the existence of electrons in 1897, he went on to propose the plum pudding model of matter. What was the plum pudding model? What did Ernest Rutherford conclude about the structure of matter based on his experimental results from bombarding gold foil with alpha particles? (b) What was the proposed atomic model of matter put forward by Rutherford? Theoretically what was the problem with his proposed model of the atom? (c) What was the modification made by Niels Bohr to Rutherford's model, i.e., what were the assumptions that Bohr made for his version of the atomic model of matter? (d) What observational phenomena was Bohr's proposed model able to explain? How did his model explain these phenomena? (e) Draw an energy level diagram with one representative transition to support your answer to part (d).

2.40 moles of an ideal gas is initially at 40.0 oC and 1.35 atm. a) What is its volume under these conditions?b) If it is then compressed to one third of its initial volume and its pressure increases to 2.0 atm, what, in Centigrade degrees, will be its temperature?

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